Answer:
The rate constant for a second order reaction is
k = 0.51 dm-3 s-1.
Explanation:
In a regular second-order reaction the rate equation is given by v = k[A][B], if the reactant B concentration is constant then v = k[A][B] = k'[A], where k' the pseudo–first-order rate constant = k[B].
Also 1/|A| = Kt + 1/|Ao|
But Ao = 0.657 M and
A = 0.0981 M also
t = 17.0 s
Therefore
1/| 0.0981 M| =K × 17.0 s + 1/| 0.657 M|
→ 10.19/M = 17K + 1.52/M
10.19/M - 1.52/M = 8.67/M = 17K
K = 8.67M/17s = 0.51 dm-3 s-1.
k = 0.51 dm-3 s-1.
